C3H8(g) +4 Cl₂(g) → C3H4Cl4(g) + 4 HCl(g) -> A 6.0 mol sample of C3H8(g) and a 20. mol sample of Cl₂(g) are placed in a previously evacuated vessel, where they react according to the equation above. After one of the reactants has been totally consumed, how many moles of HCl(g) have been produced?

Given the following reaction and the molar masses below, what is the percent atom economy (% AE) for forming H2(g)?  Enter an answer accurate to three (3) significant figures.    Zn(s) + 2 HCl(aq) → ZnCl2(aq) + H2(g)   % AE =    Molar masses (in g mol−1):   H2, 2.02 Zn, 65.38 HCl, 36.46

Classify each chemical reaction: KOH(aq) + HBrO (aq) reaction K BrO (aq) + H₂O (1) Na Cl (aq) + AgNO3(aq) → NaNO3(aq) + Ag Cl (s) 16K (s) + S₂ (s)→ 8K₂S (s) 2CH₂CH₂CO₂H (1) + 70₂(g) → 6CO₂(g) + 6H₂O(g) ✓ 6 ✓ 7 type of reaction (check all that apply) combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition combination single replacement double replacement decomposition ✓8 X precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base precipitation combustion acid-base 9 10

Aqueous solutions barium chloride and potassium sulfate are combined.  1) Predict the products and write the balanced equation showing the states of each substance. 2) The barium chloride solution has a volume of 100.0 mL and contains 10.00 grams of barium chloride.  The molarity of the potassium sulfate solution is 0.574 moles/liter and has a volume of 100.0 mL. Determine the limiting reactant and the mass of each product in grams. 3) Determine how many grams of excess reactant remain. 4) Calculate the molarity of just the potassium ions after the reaction has finished.

4. Consider the reaction MnO2 + 4HCI→ MnCl2 + Cl2 + H2O If 86.3 L of MnO2 and 48.2L of HCl react, a) Which reagent will be used up first? Which is the limiting reagent? b) How many grams of Cla will be produced?

The balanced chemical equation for the reaction between calcium hydroxide and hydrochloric acid is: Ca(OH)2 ( aq) + 2 HC1 ( aq )→ CaCl2 ( aq ) + 2 H,0 (1) We can interpret this to mean: 1 mole of calcium hydroxide and |mole(s) of hydrochloric acid React to produce: | mole(s) of calcium chloride and |mole(s) of water

The reaction for producing glucose in plants, called photosynthesis, is   6CO2+6H2O−→−−lightC6H12O6+6O2 6CO2+6H2O→lightC6H12O6+6O2    If a plant produces 5.81 mol C6H12O6,5.81 mol C6H12O6, how many moles of CO2CO2 are needed? moles CO2CO2:

Consider the reaction: 2Al(s) + 6HCl(aq) → 2AlCl3(aq) + 3H₂(g) If a sample of 4.0 moles of Al is added to a solution containing 2.0 moles of HCI, how many moles of AICI3 are formed? O 4.0 moles 6.0 moles 0.67 moles 2.0 moles O 1.0 moles MacBook Air

Classify each chemical reaction: Reaction Cl₂(g) + 2KI (aq) → 2KCl(aq) + 1₂ (s) H₂SO₂ (aq) H₂O(l) + SO₂ (g) PbCl₂ (aq) + FeSO (aq) → FeCl₂ (aq) + PbSO₂ (s) Mg(s) + F₂ (g) → MgF₂ (s) Type choose one choose one choose one choose one X Ś

Solid copper can be produced by passing gaseous ammonia over solid copper (II) oxide at high temperatures, according to the following reaction.   NH3 (g) + CuO (s) → N2 (g) + Cu (s) + H2O (g)  Balance the reaction.